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Calculate the mass of compound (molar ma...

Calculate the mass of compound (molar mass = `256 g "mol"^(-1)` ) to be dissolved in 75 g of benzene to lower its freezing point by 0.48 K `(K_f = 5.12 K kg "mol"^(-1))`.

Text Solution

Verified by Experts

Apply the formula
`M_2 = (K_f xx w_2 xx 1000)/(Delta T_f xx w_1)`
substituting the values , we have
`256 = (5.12 kg "mol"^(-1) xx wg xx 1000 g kg^(-1) )/(0.48 K xx 75 g)`
` w = (256 xx 0.48 xx 75)/(5.12 xx 1000) g = 1.8 g `
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Calculate the mass of a compound (molar mass =256 g mol^(-1) ) to be dissolved in 75 g of benzene to lower the freezing point by 0.48 K ( K_(f) =5.12 K kg mol^(-1) )

Calculatate the mass of compound (molar mass = 256 g mol^(-1) be the dissolved in 75 g of benzene to lower its freezing point by 0 .48 k(k_(f) = 5. 12 k kg mol ^(-1) .

Knowledge Check

  • How much polystrene of molar mass 9000 g mol ^(-1) would have to be dissolved in 100 g of C_(6) H_(6) to lower its freezing point by 1.05 K ?

    A
    19.3g `
    B
    `193 g `
    C
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    D
    `77.2g`

  • 1.00 g of a non-electrolyte solute (molar mass 250 g mol^(-1) ) was dissolved in 51.2 g of benzene.If the freezing point depression constnat, K_f of benzene is 5.12 K kg "mol"^(-1) , the freezing point of benzene will be lowered by

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    0.3 K
    B
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    D
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  • 1,00 g of a non-electrolyte solute (molar mass 250 g mol^(-1) ) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K kg mol^(-1) , the freezing point of benzene will be lowered by

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